Dalton's Law question.

  • Thread starter yaho8888
  • Start date
  • #1
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Homework Statement



A sample was collected into a 1.25L tank at 752 mm Hg and analyzed. The analysis showed 92% CO2, 3.6% NO, 1.2% SO2, and 4.1% H2O by mass(key word mass). what is the partial pressure exerted by each gas.




attempt at a solution:
I know that you need to times the percent of gas in the tank by the pressure.
But I try this question so many times keep get me the wrong answer.
so please show step by step solution please.
I am have a quiz tomorrow so please teach me how to do this problem thanks.
 

Answers and Replies

  • #2
133
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This might work: assume 100g total mass sample. Then 92g is CO2, 3.6 g NO etc...

Calculate the mole of each gas with the above masses 92g CO2 = > ? mol CO2

Add up all the moles to get total moles

- mole fraction (mol CO2/total moles)is proportional to partial pressure/total pressure,
- total pressure is given in the problem.
 
  • #3
62
0
This might work: assume 100g total mass sample. Then 92g is CO2, 3.6 g NO etc...

Calculate the mole of each gas with the above masses 92g CO2 = > ? mol CO2

Add up all the moles to get total moles

- mole fraction (mol CO2/total moles)is proportional to partial pressure/total pressure,
- total pressure is given in the problem.

It dosen;t seem working!
THE ANSWER OF CO2 SHOULD BE 630MM HG
 
  • #4
133
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are you sure the % values are correct? If you add up all the numbers I get 100.9%, this could make a difference in the partial pressures
 
  • #5
62
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That's how it is on the book check thousand times!
 

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